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topic 11682

Percentage composition of copper sulfate hydrate



A discussion started in 2001 & continuing through 2017

(2001)

Q. I have a question ... If anyone can, Please, HELP ME... The percentage composition of copper sulfate hydrate?

Donna Eldenson
- New Brunswick, Canada


(2002)

A. All I know is that there is 36% H2O.

Elspeth Weldon
- Raleigh, North Carolina


 

thumbs up signCopper sulphate pentahydrate is CuSO4.5H2O. If you look up the atomic weights of Cu, S, O, and H, and multiply each by how many atoms of them are in the compound per the formula above, you'll see that Elspeth is right on!

Hi Donna. I think you may have left some words out, so we don't quite understand the question. Can you write it out fully, such that it will make complete sense please? I hate to guess, not only because I could get it wrong and mislead you, but because it is vitally important to your education that you fully understand your questions before you ask someone to answer them. If you don't know an answer, you can ask someone to help; but if you don't understand the question it is foolishness to carry on without asking your teacher to clarify it :-)

Good luck

Ted Mooney, finishing.com Teds signature
Ted Mooney, P.E. RET
finishing.com
Pine Beach, New Jersey


February 7, 2009

Q. How can I figure out the concentration (in mg/L) of Cu from copper sulphate when the concentration of CuSO4 is 3 g/L?

Derek Robinson
- Toronto, Ontario, CANADA


February 18, 2009

A. Hi, Derek. This sounds like a very easy question designed to warn you if you didn't really understand the lesson :-)

What does the formula CuSO4 mean to you? It should mean a molecule that contains an atom of Cu, an atom of Sulfur, and four atoms of oxygen. Did you understand that much? Then look up the atomic weights of these elements in the Periodic Table as we suggested. You simply divide the atomic weight of copper by the atomic weight of the whole copper sulphate molecule to learn the percentage by weight of copper in copper sulphate. Then if you have 3 g/L CuSO4, you just multiply the 3 by the percentage of Cu in CuSO4 as you just determined. Good luck.

Regards,

Ted Mooney, finishing.com
Teds signature
Ted Mooney, P.E. RET
finishing.com
Pine Beach, New Jersey


February 13, 2011

Q. Hello, can anyone please help me with these answers. Thank You

1. What is the percentage copper in copper sulfate (Cuso4)?
2. What mass of copper can be obtained from 2.34 g of Cuso4?
3. The calculated mass of copper is different from (less than) the actual mass of copper carbonate. This is likely to be because:

Andrew Q [last name deleted for privacy by Editor]
student - Bogota, Colombia


February 14, 2011

A. Hi, cousin. This is where people try to help you understand rather than doing your homework for you.

So first off, when doing chemistry you MUST take the time to always capitalize correctly or you will be hopelessly confused. Every element is represented by either a single upper case letter, or by two letters where the first is upper case and the second is lower case. "Cu", for example, means copper, but "CU" would mean carbon plus uranium, and "cu" is completely meaningless. Although someone might be able to guess that you meant "copper sulfate" when you wrote "Cuso4", you may find yourself unable to progress until you employ the discipline of always capitalizing the symbols properly.

Your first question and second questions were answered immediately above your question. If you didn't understand, please tell us what you don't understand rather than pasting it from your homework assignment. Once you have the answer to your first question, the answer to the second is obvious. Good luck!

Regards,

Ted Mooney, finishing.com
Teds signature
Ted Mooney, P.E. RET
finishing.com
Pine Beach, New Jersey



April 22, 2012

Q. I want to determine the chemical formula for a hydrate.
The hydrate is Copper(II) Sulfate or CuSO4
After conducting the experiment I found the mass percentage of this compound is:
28.4% water
71.6% copper(II) sulfate

This is how I find the number of hydrates in the solution:
CuSO4.xH2O (where x is the number of hydrates)

Assume 100 g sample

28.4 g of water, 71.6 g of copper(II) sulfate

Number of moles of water in this sample = 28.4 g/ molar mass of water (18.02 g/mol)

= 1.576 moles

Number of moles of copper sulfate in this sample = 71.6 g / (159.62 g/mol)

= 0.449

Divide by the smallest mole number to get a whole number ratio

0.449/0.449 = 1
1.576 /0.449 = 3.51

1:3.51

From here do I round up to 4 so the ratio is 1 copper sulfate molecule for every 4. Or do I multiply by 2 so I have a 2:7 ratio?

Cyrus D.
- Toronto, Ontario, Canada


April 26, 2012

A. You have two possibilities:
1. Your analyses method was not the best.
Sometimes the last water is a bit hard to drive off. Crushing the crystals will give you a lot more surface area. Weigh the powder, not the crystals.
Did you check the weigh boat after the "wet" weight to see if any remained?
You could repeat the process and see if any more water will come off. Too aggressive a drying might have driven off a tiny bit of the copper compound with the moisture (steam). Sometimes the crystals will pop like popcorn.
Is your balance accurate enough? Was it calibrated before you started?
Did you leave enough time for the temperature to equilibrate after the drying?

2. You might be working with a mixture of water of hydration.

A normal lab experiment is run in triplicate. How do your 3 runs agree?

What does your teacher think??

James Watts
- Navarre, Florida


Very informative, James, thanks!

Regards,

Ted Mooney, finishing.com
Teds signature
Ted Mooney, P.E. RET
finishing.com
Pine Beach, New Jersey


April 29, 2012

thumbs up signMy teacher told me to round to 4. And yes you are right the correct ratio is 1:5. I didn't fully heat the compound so I guess that's just going to be my source of error!

Thanks

Cyrus D.
- Toronto, Ontario, Canada



October 16, 2017

Q. How do I calculate the mass of 2 moles of copper sulphate crystals CuSO4.8H2O

Geeta saini
- London, West Drayton,UK


wikipedia
Mole (unit)
October 2017

Hi Geeta. Are you sure you understand what a mole is? That's certainly step 1 :-)

Mole is short for "gram molecular weight"; so one mole of any element or compound weighs (in grams) whatever is the atomic weight of all of the constituents in the molecule. So a mole of CuSO4.8H2O weighs (in grams) one atomic weight of copper, plus one atomic weight of sulfur, 12 atomic weights of oxygen, and 16 atomic weights of hydrogen.

Two moles weighs roughly 1.999 times as much. Good luck.

Regards,

pic of Ted Mooney
Ted Mooney, P.E. RET
finishing.com
Pine Beach, New Jersey
Striving to live "Aloha"



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